I can't believe I really have to go back and take this final during my summer.
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| matter | anything that has a mass and occupies space
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| element | basic substances that make up all of the matter in our world
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| atom | infinitesimally small building blocks of matter
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| molecule | two or more atoms are joined together in specific shapes
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| mixture | combinations of two or more substances in which each substance retains its own chemical identity
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| pure substance | matter that has a distinct property and a composition that doesn't vary from sample to sample
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| compound | substances composed of two or more elements, so they contain two or more kinds of atoms.
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| intensive property | a property that does not depend on the amount of the sample being tested (BP, Density)
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| extensive property | a sample that does depend on the quantity of the sample (mass, volume)
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| physical property | can be measured without changing the identity and composition of the sutace (color, odor)
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| chemical property | describe the way a substance may chane or react to form other substances (flammability)
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| mass | a measure of the amount of material in an object. (kg ~ 2.2 lbs)
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| temperature | a measure of the hotness or coldness of an object.
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| density | a property of matter defined as the amount of mass in a unit volume of the substance D=M/V
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| precision | a measure of how closely individual measurements agree with one another
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| accuracy | how closely individual measurements agree with the correct value
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| converstion factor | a fraction whose numerator and denominator are the same quantity expressed in diferent units
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| C --> F | F = 9/5(C)+32
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| F --> C | C= 5/9(F-32)
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| C --> K | K = C = 273.15
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| subatomic particles | what the atom is composed of
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| proton | resides in the nucleaus of the atom, charge is +1
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| electron | have a charge of -1
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| neutron | resides in nucleus of atom, has no charge
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| isotope | atoms with identical atomic numbers but diferent mass numbers
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| atomic number | number of protons in the nucleus of an atom
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| atomic weight | avg atomic mass of each element
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| periodic table | arangement of elements in order of increasing atomic bumber with elements having similar properties plaed in vertical columns
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| matallic elements | left & middle of PT share prprerties suchas luster and high electrical and heat conductivity, solids at room temp.
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| nonmetallic elements | room temp some are gaseous, some solid, one liquid. different in appearance and other properties
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| metalloids | in the way of properties, these fall between metals and nonmetals
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| groups (families) | vertical columns of periodic table
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| transition elements | transition elements
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| diatomic | a molecule that is made up of two atoms
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| molecular formulas | chemical formulas that indicate actual numbers and types of atoms in a molecule
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| empirical formulas | chem formulas that give only the relative number of atoms of each type in a molecule
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| molecular compounds | compounds that are composed of molecules
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| ionic compounds | a coumpound that contains both negatively and positively charged ions
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| monoatomic ions | simpler ions
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| polyatomic ions | consist of atoms joined as in a molecule, but have a net positive or negative charge
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| anion | negatively charged ion
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| cation | positively charged ion
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| stoichiometry | examines quantities of sustances consumed and preduced in chemical reacions
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| law of conservation of mass | states that mass can neither be created or destroyed
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| chemical equation | the consise way in which chemical reactions are created
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| combination reaction | two or more substances react to form one product
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| decomposition reaction | one substance undergoes a reaction to produce two or more other substances
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| combustion reaction | rapid reactions that produce a flame. most involve O2 from air as a reactant
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| formula weight | sum of the atomic weights of each atom in its chemical formula.
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| molecular weight | total weight of a molecule
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| percentage compostion | percentage by mass contributed by each element in the substance
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| mole | amount of matter that contains as many objects as the number of atoms in exactly 12g of isotopically pure 12C.
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| avogardos number | 6.022 x 10^23
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| molar mass | mass in grams of one mole of the substance
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| empirical formula | tells us relative number of atoms of each element it contains
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| molecular formula | always a whole number multiple of the corresponding subscripts of the empirical formula
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| limiting reactant | the reactant in a reaction that is completely consumed, thus controlling when the reacton stops
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| theoretical yield | quantity of product that is calculated to form when all of the limiting reactant reacts
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| aqueous solution | solutions in which water is the dissolving medium
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| strong electrolyte | solutes that exist in solution completely or nearly completely as ions
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| weak electrolyte | solutes that exist in the solution mostly in the form of molecules with only a small fraction in the form of ions
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| nonelectrolyte | a substance that does not form ions in solutions
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| molecular compounds in water | usually consists of intact molecules dispersed throughout the solution. Most molecular compounds are nonelectrolytes.
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| ionic compounds in water | ions are separated by the H2O molecules and solvated which helps stabilize the ions in solution and prevents cations and anions from recombining.
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| precipitation reactions | reactions that result in the formation of an insoluble product.
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| solubility | the amound of substance that can be dissolved in a given quantity of solvent at that temperature
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| chemical equilibrium | the balance between opposing processes that determines the relative numbers of ions and neutral molecules.
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| exchange (metathesis) reactions | reactions in which positive ions and negative ions appear to exchange partners conform to the following general equation : AX + BY --> AY + BX
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| complete ionic equation | an equation written with all soluble strong electrolytes shown as ions
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| net ionic equation | whats left when spectator ions are eliminated
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| spectator ions | ions that appear in identical forms in both the reactants and products of an equation
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| acid | substances that ionize in aqueous solutions to form H ions, thereby increasing the concentration of H ions.
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| acid/base reactions (neutralization) | produces a water and a salt
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| oxidation | loss of electrons by a substance
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| reduction | gain of electrons by a substance
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| redox reactions | oxidation-reduction; electrons are transferred between reactants.
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| activity series | a list of metals arranged in order of decreasing ease of oxidation
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| concentration | the designated amount of solute dissolved in a given quantity of solvent or quantity of solution
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| molarity | concentration of a solution as the number of moles of solute in a liter of solution
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| dilution of stock solutions | by adding water to a concentrated stock solution, you can obtain a solution of lower concentration.
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| titration | combining a sample of the solution with a reagent solution of known concentratino to find out the concentration of a particular solute in a solution
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| equivalence point | the point at which stoichiometrically equivelent quantities are brought together
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| indicator | a substance added to a solution to indeicate by a color change the point at which the added solute has reacted with all the solute present in the solution
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| base | substances that accept H+ions. produce OH- ions when dissolved in water
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| I- | Iodide
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| HI | Hydroiodic Acid
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| IO2- | iodite
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| IO3- | Iodate
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| IO4- | Periodate
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| CO3(2-) | Carbonate
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| SO4(2-) | Sulfate
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| NO3- | Nitrate
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| H2CO3 | Carbonic Acid
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| H2SO4 | Sulfuric Acid
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| HNO3 | Nitric Acid
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| S(2-) | Sulfide
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| NO2- | Nitrite
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| HNO2 | Nitrous Acid
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| For a metal to be a cation it must _ electrons | lose
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| For a nonmetal to become an anion it must _ electrons | Gain
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| Ca3N2 (comp.) | Calcium Nitride
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| NO2 (comp.) | Nitrogen Dioxide
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| Cu2SO4 | Copper (I) Sulfate
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| Al2S3 | Aluminum Sulfide
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| Na2CO3 | Sodium Carbonate
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| Iron (III) Sulfide | Fe2S3
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| Phosphorous Trioxide | PO3
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| Ammonium Chloride | NH4Cl
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| Magnesium Nitrite | Mg(N02)2
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| Sodium Hypochlorite | NClO
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| sp3 hybridization in the carbon atom | one s orbital is hybridized with 3 p orbitals creating 4 new orbitals whose energy is less than p but more than s
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| sp Hybridized C atom | Sigma bonds? = 2P orbital? = 2Pi bonds? = 2total bonds? 4
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| alpha particle | 4/2He
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| beta decay | electron. (0/-1 e)
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| positron | positive electron (0/+1e)
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| half life | how long it takes for something to be half way used up. K=.693/half life then ln(Nt/No)= -KT
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| rad and rem. beter to use in measuring exposure a technician has experienced & why? | Rem is better. It incorporates Rad into it. rem measures how much damage the absortion has done and what kind of rad exposure.
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| fission/fusion, which is used today | fission is splitting of an atom into two smaller atoms. Fusion is the comination of two atoms. fission is used because fusion must be done at ridiculously high temperatures.
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| trend for atom size in IA metals. How does each compare to its parent atom | Atom size decreases down the PT. Ions are smaller than parent atoms
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| electron affinity increases across PT (L to R). Why? | the farther right you go the fewer electrons the element needs, so the electron affinity increases.
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| difference in ionization energy and electron affinity? | IE is the amount of energy required to remove and electron, while electron affinity refers to the energy needed to gain an electron. The higher the electron affinity the more an element has nonmetallic characteristics.
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| STP | 760mmHg, 1atm
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| Pressure | conveys the idea of a force, a push that tends to move something in a given direction. P is the Force that acts on a given Area ( P = F/A )
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| Temperature |
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| Boyle's Law | the volume of a fixed quantity of gas maintained at constant temperature is inversely proportional to the pressure. PV = Constant
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| Charles' Law | the volume of a fixed amount of gas maintained at constant pressure is directly proportional to its absolute temperature V/T = Constant.
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| Avogadro's Hypothesis | equal vlumes of gases at the same temperature and pressure contain equal numbers of molecules.
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| Avogadro's Law | the volume of a gas maintained at constant temperature and pressure is directly proportional to the number of moles of gas. V= Constant(n)
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| Combined gas law equation |
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| ideal gas equation | PV = nRT, P1V1 = P2V2
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| gas constant | the term R in the ideal gas equation.
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| daltons law of partial pressures | the total pressure of a mixture of gases equals the sum of the pressures hat each would exert if it were present alone. Pt = P1 + P2 + p3...
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| mole fraction | ratio n1/n2. a dimensionless number that expresses the ratio of the number of moles of one component to the total number of moles in the mixture.
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| kinetic molecular theory | a model that helps us picture what happens to gas particles as experimental conditions such as pressure or temperature change
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| effusion | escape of gas molecules through a tine hole one molecule at a time
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| diffusion | spread of one substance throughout a space or throughout a second substance
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| Graham's law of effusion | R1/R2= Square root of MW2/MW1
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| thermodynamics | the study of energy and its formations
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| kinetic energy | the energy of motion
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| potential energy | can possess this by virtue of its position relative to other objects
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| system | portion singled out for study
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| surroundings | everything but the system
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| work | energy used to cause an object with mass to move
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| force | any kind of push or pull exerted on an object
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| heat | the energy used to cause the temperature of an object to increase
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| thermal energy |
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| energy | the capacity to do work or transfer heat
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| first law of thermodynamics | energy is conserved
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| endothermic | the system absorbs heat
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| exothermic | the system releases heat
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| state-function | a property of a system that is determined by specifying the systems condition or state; depends only on present state of system
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| pressure volume work | the wrok involved in expansoin or compression of a gas
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| enthalpy | accounts for heat flow in processes occuring at constant pressurewhen no forms of work are performed other that PV work.
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| enthalpy of reaction | the enthalpy change that accompanies a reaction
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| calorimetry | the measurement of heat flow
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| heat capacity | the amount of heat required to raise its temperature by 1K
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| molar heat capacity | the heat capacity of one mole of a substance
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| specific heat | heat capacity of one gram of a substace
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| bomb calorimeter | a device that helps with the study of combustion reactions
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| enthalpy of formation | enthalpy change associated with a proces that forms a compound from its constituent elements
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| standard enthalpy of formation | change in enthalpy for the reaction that forms one mole of the compund from its elements
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| fuel value | the energy released when one gram of a material is combusted
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| fossil fuels | fuel such as coal petroleum and natural gas which have formed over millions of years ago rom decompostion of plants and animals
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| renewable energy and examples | energy sources that are essentially inexhaustable
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| electronic structure | the arrangement of electrons in atoms
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| electromagnetic radiation | light we can see with our eyes
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| wavelength | distance between two adjacent peaks
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| frequency | number of complete wavelengths
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| quantum | smallest quantity of energy that can be emitted or absorbed as electromagnetic radiation.
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| photons | an individual energy packet
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| spectrum | radiation separated into different wavelengths
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| continuous spectrum | spectrum containing all wavelengths
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| line spectrum | spectrum containing radiation of only specific wavelengths
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| ground state | lowest energy state
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| excited state | highest energy state
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| uncertainty principle | heisenbergs principle
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| orbitals | defines a specific distribution of electron density in space.
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| electron shell | colection of orbitals with the same value of n
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| subshell | set of orbitals with same n and l values
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| electron configuration | the way electrons are distributed among the various oritals of an atom
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| valence electrons | outer shell electrons -- used in binding with other electrons
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| core electron | iner shell electrons
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| representative elements | s and p block together
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| transition elements | middle elements
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| lanthanide series | top row of F block metals
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| actinide series | final row of PT
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| f-block metals | all the underneath rows in the PT
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| electromagnetic spectrom | wavelength --->gamma, x, ultraviolet, visible, ingrared, micro, radio<---frequency
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| metallic character | the more an element exhibits the physical and chemical properties of a metal, the greater its metallic character. metals tend to hav elow ionization energies and therefore tend to form positive ions relatively easily
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| nonmetallic character | vary greatly in appearance
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| alkali metals | soft metallic solids. silvery, high thermal and electrical conductivities.
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| alkaline earth metals | harder and more dense and melt at higher temps than alkali metals.
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| halogens | salt formers. nonmetals. melting and BPs increase with increasing atomic number
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| noble gases | all nonmetals that are gases at room temperature. all monatomic.
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| chemical bond | two atoms or ions strongly attached to each other
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| ionic bond | eletrostatic forces that exist between ions of opposite charge.
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| covalent bont | sharing of electrons between two atoms
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| metallic bond | found in matals. each atom in a metal is bonded to several neighboring atoms
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| octet rule | atoms tend to gain lose or share electrons until they are surrounded by eight valence electrons.
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| lewis symbol | consists of chemical symbol of element plus a dot for each valence electron
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| bond polarity | describes the sharing of electrons between atoms
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| nonpolar covalent bond | one in which the electrons are shared queally between two atoms.
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| polar covalent bond | one of the atoms exerts a greater attraction for the bonding electrons taht the other
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| electronegativity | the ability of an atom in a molecule to attract electrons to itself
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| formal charge | charge the atom would have if all the atoms in the molecule had the same electronegativity.
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| resonance structure | placement of electrons is differernt than in lewis structures
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| sigma bonds | end on overlap
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| pi bonds | sidways overlap
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| vsepr | valence shell electron particle repulsion
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| nucleons | subatomic particles that reside in the nucleus
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| radionuclides | nuclei that are radioactive
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| radioisotopes | atoms containing radionucleides
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| gamma radiation | high energy photons. represented as 0/0y.
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| electron capture | capture by the nucleus of an electron from the electron cloud surrounding the nucleus.
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| belt of stability | above, beta particle emission. below, positron emission or electron capture.
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| radioactive series | a series of nuclear reactions that begins with an unstable nucleus and terminates with a stable one
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| nuclear transmutations | when a nucleus changes its identity because its struck by a neutron or another neucleus
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| particle accelerators | atom smashers
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| transuranium elements | they occur immediately following uranium in the periodic table
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| geiger counter, | detects and measures radioactivity
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| chain reactions | reactions that multiply
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| critical mass | amount of fissionable material large enough to maintain the chain reaction with a constant rate of fission
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| supercritical mass | a mass in excess of a critical mass
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| control rod | regulate flux of neutrons to keep the reation chain self sustainingwhile preventing the reactor core from overheating
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| moderator | slows down neutrons so they can be more readily absorbed by the fuel
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| ioniing radiation | radiation that causes ionization, far more damazing
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| non ionizing radiation | generally of a lower energy.
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| free radical | unstable and highly reactiv OH molecule.
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| gray | SI unit of absorbed dose.
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Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
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To hide a column, click on the column name.
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